Chemistry Elements Quiz

Questions and Answers

What are group 1 elements?

Alkali metals

What are group 2 elements?

Alkaline earth metals

What are group 3-12 metals?

Transition metals

What are the elements along the zig-zag or in between the metals and nonmetals?

Metalloids Signup and view all the answers

What group is 17 or 7A?

Halogens Signup and view all the answers

What group is 18 or 8A?

Noble gases Signup and view all the answers

What are the elements at the bottom of the periodic table?

Inner transition elements Signup and view all the answers

What are metals?

Elements containing atoms that readily lose electrons to form positive ions (cations) Signup and view all the answers

What are the chemical properties of metals?

Few electrons in the valence energy level, lose electrons readily, positive charge, form cations Signup and view all the answers

What do the group numbers also represent?

Number of valence electrons Signup and view all the answers

What are physical properties of metals?

Ductile, malleable, high tensile strength, good conductors of heat and electricity, luster, mostly solid at room temperature Signup and view all the answers

Which metal is not a solid at room temperature?

Mercury Signup and view all the answers

Most metals have _____________ valence electrons. Valence electrons are easily _, making some metals _______________.

one or two; lost; very reactive Signup and view all the answers

All alkali metals have ____ valence electron.

one Signup and view all the answers

Alkali metals are _ found in pure form in nature; they are too ____.

never; reactive Signup and view all the answers

Reactivity ______________ down the group. Are alkali metals very reactive?

increases; YES, they are the most reactive. Signup and view all the answers

What are some physical properties of alkali metals?

Soft, silvery in color Signup and view all the answers

All alkaline earth metals have ______ valence electrons.

two Signup and view all the answers

Alkaline earth metals are _______ reactive than alkali metals.

less Signup and view all the answers

Alkaline earth metals are _ found in a pure form in nature; they are too ___________.

not; reactive Signup and view all the answers

What does the word alkaline mean?

Basic Signup and view all the answers

What are nonmetals?

Elements containing atoms that readily gain electrons to form negative ions (anions) Signup and view all the answers

What are chemical properties of nonmetals?

Almost full or full valence energy levels, tend to gain electrons, negative charge, form anions Signup and view all the answers

What are physical properties of nonmetals?

Not ductile, not malleable, bad conductors, brittle, mostly solid, some are gases at room temperature Signup and view all the answers

Which nonmetal is liquid at room temperature?

Bromine Signup and view all the answers

Nonmetals have a ____________________________ valence energy level. Electrons are easily _ by elements with nearly full outer energy levels making them very _________.

a full or almost full; attracted; reactive Signup and view all the answers

Halogens have _ valence electrons. Halogens are the most group of nonmetals. Halogens are only found in a pure form as a ___ element.

7; reactive; diatomic Signup and view all the answers

Noble gases have __ valence electrons (full outer energy level) except helium that has _ valence electrons.

8; 2 Signup and view all the answers

Noble gases are chemically ___________ and are only found in pure form in nature. They are _ and ________.

unreactive; colorless; odorless Signup and view all the answers

What are the chemical properties of metalloids?

Form anions or cations depending on the environment, have properties of both metals and nonmetals Signup and view all the answers

What are the physical properties of metalloids?

Semi-conductors, some metalloids have metallic luster, metalloids are semi-conductors of electricity, some are gases at room temperature Signup and view all the answers

What do p-block elements contain?

All nonmetals except hydrogen and helium. Contains six metalloids. Contains 12 metals. Signup and view all the answers

P-block and s-block elements make up the __________________ elements.

Main group Signup and view all the answers

Properties of the p-block __________ greatly.

Vary Signup and view all the answers

Which Russian chemist was the first to publish a system classifying elements in 1869?

Dmitri Mendeleev Signup and view all the answers

What is always the same no matter what language the Periodic Table is published in?

Element symbols Signup and view all the answers

What did Mendeleev do that finally convinced scientists that his table worked?

Predicted properties of elements that would fill 3 empty spaces Signup and view all the answers

What were two problems with Mendeleev's Periodic Table?

Iodine and Tellurium (didn't organize by property), Noble gases had not been discovered Signup and view all the answers

In what order did Mendeleev organize the elements known at his time?

Atomic number Signup and view all the answers

Henry Moseley in 1911 was credited for what three things regarding the periodic table?

Elements fit into patterns better by atomic number, the atomic number, periodic law Signup and view all the answers

What is the periodic law?

The physical and chemical properties of the elements are the periodic functions of their atomic numbers. Signup and view all the answers

What does periodically mean?

At certain intervals Signup and view all the answers

There are ____ naturally occurring elements.

92 Signup and view all the answers

All elements in the same period have the same number of

Principle energy levels Signup and view all the answers

Elements are also arranged vertically in the periodic table in ___ that share similar _ __________.

Groups; chemical properties Signup and view all the answers

Elements in groups have the same number of . And therefore lose or gain the same number of electrons when forming ions.

Valence electrons Signup and view all the answers

Inner levels of electrons _____ the outer (valence) electrons blocking the _ ________ on these electrons.

Repel; nuclear effect Signup and view all the answers

Going down the group, shielding ________________ with the addition of more energy levels.

Increases Signup and view all the answers

The hold on the valence electrons by the _________________ is weakened causing the electrons to become easier to remove.

Nucleus Signup and view all the answers

Why is the most reactive nonmetal fluorine?

With very little shielding, the positive nucleus pulls the fluorine atom in closely, making it very easy to attract an 8th electron to its outer energy level. Signup and view all the answers

What is atomic radius?

One half of the distance between the nuclei of identical atoms that are bonded together Signup and view all the answers

How is atomic radius measured?

Picometers (pm) or angstroms (A); an angstrom is $1 \times 10^{-10}$ Signup and view all the answers

What is the periodic trend of atomic radius?

Atomic radius decreases going across the period but increases going down the group Signup and view all the answers

The number of protons increasing in the nucleus while going across a period increases the _.

Positive nuclear charge Signup and view all the answers

What does an increase in positive nuclear charge do to an atom?

Attracts electrons towards the nucleus making atoms smaller Signup and view all the answers

Moving down a group, each new period adds another energy level. Each level is from the __ and increases the atomic radius.

Further; nucleus Signup and view all the answers

Positive ions are ___________ than the neutral atom from which they are formed.

Smaller Signup and view all the answers

Valence electrons are removed. More protons than electrons cause the _____________ to 'pull' in electrons closer.

Nucleus Signup and view all the answers

The resulting cation is smaller than the ______________ atom.

Neutral Signup and view all the answers

Negative ions are ____________ than the neutral atom from which they are formed.

Larger Signup and view all the answers

The extra _ produced from the additional electrons cause the ion to ____.

Repulsion; expand Signup and view all the answers

Valence electrons are added. More electrons than protons cause the ion to __________ due to repulsive forces.

Expand Signup and view all the answers

What is ionization energy?

The energy required to remove an electron from an atom Signup and view all the answers

What is the periodic trend for ionization energy?

Ionization energy increases across the period. As the atomic radius decreases, valence electrons are held closer to the nucleus. Signup and view all the answers

What is the group trend for ionization energy?

Ionization energy decreases down the group. As the atomic radius increases, it becomes easier to remove valence electrons. Signup and view all the answers

Describe first ionization energy.

The energy needed to remove an outermost electron. Signup and view all the answers

Why is the second ionization energy for sodium so much higher than the first?

It requires more energy to remove an electron from a cation than a neutral atom. Signup and view all the answers

Why is there a lower ionization energy for elements further down the group?

The outermost electron is on average farther from the nucleus and it is held less tightly. Signup and view all the answers

What is electronegativity?

A measure of the ability of an atom in a chemical compound to attract electrons from another atom. Signup and view all the answers

What is the periodic trend for electronegativity?

Electronegativity increases across the period. The increasing positive nuclear charge allows atoms to attract electrons more effectively. Signup and view all the answers

What is the group trend of electronegativity?

Electronegativity decreases down the group. The increase in atomic radius reduces the effective force attracting electrons. Signup and view all the answers

Why does electronegativity increase across the period?

The number of charges on the nucleus increases. Signup and view all the answers

Which has a smaller atomic radius, Ca or Ca^2+?

Ca^2+ is smaller because a cation is larger. Signup and view all the answers

Which has a smaller atomic radius, F or F-?

F because anions swell. Signup and view all the answers

What is shielding?

Inner levels of electrons repel the outer (valence) electrons blocking the nuclear effect on these electrons. Signup and view all the answers

How many valence electrons in group 17?

7 Signup and view all the answers

Why does atomic radius decrease going across the period left to right on the periodic table?

Across a period, the atomic size decreases as the number of shells remains the same, but the nuclear charge increases. Signup and view all the answers

Are cations or anions larger?

Anions, more electrons Signup and view all the answers

Which element is the most electronegative?

Fluorine Signup and view all the answers

Do metals have high electronegativity?

Since metals have few valence electrons, they tend to increase their stability by losing electrons to become cations. Consequently, the electronegativities of metals are generally low. Signup and view all the answers

Study Notes

Group Elements

Group 1 elements are known as alkali metals.
Group 2 elements are identified as alkaline earth metals.
Transition metals, also referred to as B group or D block elements, are located in groups 3-12 and exhibit metallic properties.
Metalloids are the elements situated along the zigzag line between metals and nonmetals.

Group Characteristics

Group 17, or 7A, elements are termed halogens.
Group 18, or 8A, elements are recognized as noble gases.
The inner transition elements include lanthanides (6th period) and actinides (7th period), classified as f-block elements.

Metals and Their Properties

Metals are characterized by their ability to lose electrons easily, forming positive ions known as cations.
They typically have 1 or 2 valence electrons, making them reactive.
Chemical properties of metals include losing electrons readily, resulting in a positive charge.
Physical properties include ductility, malleability, high tensile strength, good electrical and thermal conductivity, and typically a shiny luster; most are solid at room temperature, except for mercury.

Reactivity Trends

Reactivity tends to increase down the group for alkali metals, making them the most reactive group of metals.
All alkali metals have one valence electron, while alkaline earth metals have two and are less reactive.

Nonmetals and Their Properties

Nonmetals are elements that tend to gain electrons, forming negative ions or anions.
They possess nearly full valence energy levels, leading to a tendency to gain electrons, resulting in negative charges.
Physical properties include being non-ductile, poor conductors of electricity, brittle, and many being gases at room temperature; bromine is the only liquid nonmetal at room temperature.

Halogens and Noble Gases

Halogens possess 7 valence electrons and are known to be very reactive nonmetals, usually found as diatomic molecules in nature.
Noble gases have 8 valence electrons, except for helium, which has 2. They are chemically unreactive, colorless, and odorless.

Periodic Table Insights

Dmitri Mendeleev is credited with the first systematic classification of elements based on atomic mass.
Mendeleev’s periodic law suggests that properties of elements are periodic functions of their atomic numbers.
The periodic table consists of 92 naturally occurring elements and organizes elements into periods (rows) and groups (columns).

Atomic Properties

Atomic radius is defined as half the distance between the nuclei of identical bonded atoms. It decreases across a period and increases down a group due to the increasing nuclear charge.
Ionization energy represents the energy required to remove an electron from an atom, which generally increases across a period and decreases down a group due to atomic size.

Electronegativity Trends

Electronegativity measures an atom's ability to attract electrons; it increases across a period and decreases down a group.
Fluorine is the most electronegative element, while metals typically have low electronegativity due to their tendency to lose electrons.

Ions and Their Sizes

Cations are smaller than their parent atoms due to the loss of valence electrons and increased nuclear pull.
In contrast, anions are larger than their parent atoms, as the addition of electrons leads to increased repulsion among electron configurations.

Additional Concepts

Shielding refers to the effect where inner electrons repel outer electrons, which affects the nuclear force experienced by valence electrons.
The periodic behavior of elements involves recognizing the trends in reactivity, size, ionization energy, and electronegativity across periods and groups in the periodic table.

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Description

Test your knowledge on the different groups of elements in the periodic table with this quiz. From alkali metals to metalloids, challenge yourself to remember their definitions and properties. Perfect for chemistry students wanting to review essential concepts.